Chapter 2-Water And Carbon: The Chemical Basis Of Life

Front 1

4 types of atoms

Back 1

hydrogen, carbon, nitrogen, and oxygen

Front 2

Protons

Back 2

Positively charges particles

Front 3

Neutrons

Back 3

Neutral particles

Front 4

Electrons

Back 4

Negatively charged particles

Front 5

Where are protons and neutrons located?

Back 5

In the nucleus

Front 6

Orbitals

Back 6

It is the spherical region around an atomic nucleus in which an electron is present most of the time. Each can hold up to two electrons. They are grouped into levels called electron shells, smaller numbers are closer to the nucleus

Front 7

Electron shell

Back 7

A group of orbitals of electrons with similar energies. Electron shells are arranged in roughly concentric layers around the nucleus of an atom, with outer shells having more energy than those in inner shells. Electrons in the outermost shell, the valence shell, often are involved in chemical bonding. each contains a specific number of orbitals, with a single orbital being able to hold two electrons. The innermost shell is filled to the outermost.

Front 8

Atomic Number

Back 8

Each atoms specific number of protons that they have in the nucleus. The bottom number on the periodic table.

Front 9

Element

Back 9

A substance, consisting of atoms with a specific number of protons, that cannot be separated into or broken down into any other substance. They preserve their identity in a chemical reaction. Atoms that have the same atomic number have the same chemical properties and belong to the same element.

Front 10

Isotopes

Back 10

Any of several forms of an element that have the same number of protons but differ in the number of neutrons

Front 11

Mass number

Back 11

The sum of the protons and neutrons in the most common isotope. the top number in the periodic table

Front 12

Chemical Bonds

Back 12

An attractive force binding two atoms together. Covalent bonds, ionic bonds and hydrogen bonds are all chemical bonds.

Front 13

Covalent Bond

Back 13

Two atoms share one or more pairs of electrons. Substances that hold them together are molecules.

Front 14

Ionic Bond

Back 14

Electrons are transferred from one atom to another.

Front 15

Electronegativity

Back 15

A measure of the ability of an atom to attract electrons toward itself from an atom to which it is bonded.

Front 16

Nonpolar covalent bond

Back 16

A covalent bond in which electrons are shared equally between two atoms of the same or similar electronegativity

Front 17

ion

Back 17

An atom or molecule that carries a charge

Front 18

Cation

Back 18

An atoms that loses an electron and becomes positively charged.

Front 19

Anion

Back 19

An atom that gains an electron and becomes negatively charged

Front 20

Ionic bond

Back 20

chemical bond that is formed when an electron is completely transferred from one atom to another so that the atoms remain associated due to their opposite electric charges

Front 21

molecular formulas

Back 21

a notation that indicates only the number and types of atoms in a molecule

Front 22

structural formulas

Back 22

A 2-D notation in which the chemical symbols for the the constituent atoms are joined by straight lines representing single, double, or triple covalent bonds.

Front 23

Which models show 3-D models

Back 23

Ball and Stick and Space Filling Models.

Front 24

When do chemical reactions occur?

Back 24

1. One substance is combined with another.
2. One substance is broken down into another substance
***In most cases, chemical bonds are broken down and new bonds form

Front 25

Molecular weight

Back 25

the sum of the mass of all of the atoms in a molecule; roughly the total number protons and neutrons in the molecule

Front 26

Mole

Back 26

6.022 X 10 to the 23. It has a mass equal to the molecular weight expressed in grams.

Front 27

Molarity

Back 27

the number of moles per liter

Front 28

Properties of water

Back 28

1. adhesive
2. cohesive
3. denser as a solid than as a liquid
4. able to absorb large amounts of energy

Front 29

Cohesion

Back 29

the tendency of certain like molecules to cling together due to attractive forces, which results in surface tension

Front 30

Surface Tension

Back 30

the cohesive force that causes molecules at the surface of a liquid to stick together, therby resisting defrormation of the liquids surface and minimizing its surface area

Front 31

Adhesion

Back 31

binding between two unlike molecules

Front 32

Specific Heat

Back 32

a measure of the capacity of a substance to absorb energy

Front 33

Heat of vaporization

Back 33

the energy required to vaporize 1 gram of a liquid to a gas

Front 34

pH

Back 34

A measure of the concentration of protons in a solution and thus if acidity or alkalinity. defined as the negative of the base -10 log of the proton concentration: pH=
-log [H+]. Acids have a pH of less than 7, bases greater than 7. water has a pH of 7.

Front 35

Acid base reactions

Back 35

A proton donor (acid) transfers a proton to a proton acceptor (base)

Front 36

Buffers

Back 36

a substance that, in solution, acts to minimize changes in the pH of that solution when acid or base is added.

Front 37

Chemical Equilibrium

Back 37

A dynamic but stable state of a reversible chemical reaction in which the foreward and reverse reactions proceed at the same rate, so that the concentrations of reactants and products remain constant

Front 38

Endothermic reactions

Back 38

Must absorb heat to proceed

Front 39

Exothermic Reactions

Back 39

Release heat during the reaction

Front 40

Energy

Back 40

the capacity to do work or supply heat. may be stored (potential) or available in the form of motion (kinetic)

Front 41

Potential Energy

Back 41

energy stored in matter as a result of its position or molecular arrangement

Front 42

Kinetic Energy

Back 42

the energy of motion

Front 43

thermal energy

Back 43

the kinetic energy of molecular motion. AKA temperature

Front 44

First law of thermodynamics

Back 44

the principle of physics tat energy is conserved in any process. Energy can be transferred or and converted into different forms, but it cannot be created nor destroyed

Front 45

factors that make a rxn spontaneous

Back 45

1. the amount of potential energy
2. the degree of order

Front 46

Entropy

Back 46

A quantitative measure of the amount of disorder in any system

Front 47

Second law of thermodynamics

Back 47

the principle of physics that the entropy of the universe or any closed system increases during any spontaneous process.

Front 48

Gibbs Free energy change.

Back 48

A measure in the change in potential energy and entropy that occurs in a given chemical reaction.

Front 49

Exergonic reaction

Back 49

referring to a chemical reaction that can occur spontaneously, releasing heat and/or increasing energy

Front 50

Endergonic reaction

Back 50

referring to a chemical reaction that requires an input of energy to occur

Front 51

Photons

Back 51

a discrete packet of light energy; a particle of light

Front 52

free radicals.

Back 52

any substance containing one or more atoms with an unpaired electron. Unstable and and highly reactive. Formed when photons come in and break molecules apart by knocking electrons away from the valence shell

Front 53

Chemical Energy

Back 53

the potential energy stored in covalent bonds between atoms.

Front 54

Amino and carboxyl group

Back 54

Attract or drop a proton

Front 55

Carbonyl group

Back 55

sites of reaction that link molecules into larger, more complex compounds

Front 56

hydroxyl group

Back 56

Act as a weak acid

Front 57

Phosphate group

Back 57

has two negative charges